AP EAMCET · Chemistry · Electrochemistry

For ${Cr}_{2} O_{7}^{2 -} + 14 H^{+} + 6 e^{- yields} ⟶ 2 {Cr}^{3 +} + 7 H_{2} O, E^{0} = 1.33 V$ at $[{Cr}_{2} O_{7}^{2 -}] = 4.5$ millimole, $[{Cr}^{3 +}] = 1.5$ millimole and $E = 1.067 V$ , then calculate the $pH$ of the solution.

A $2$
B $3$
C $2.5$
D $1.5$

Verified Solution

Answer & Solution

Correct Answer

(A) $2$

Step-by-step Solution

Detailed explanation

According to the Nernst's equation: E = E°-RTnFlnQ So, by given value of concentrations the above formula can be modified as E = E°-0.059nFlogCr3+2Cr2O72-H+14 1.067 = 1.33-0.066×96500log15×10-324.5×10-3H+14…

Apply the relevant identity from the chapter and substitute the values established in the previous step, keeping the original constraint in view.

Use the simplified expression to isolate the unknown, then plug the result back into the question setup to confirm the working is internally consistent.

Cross-check against a boundary or limiting case. Both the dimensional balance and the qualitative behaviour at the extreme should agree with the candidate answer.

Combine the steps above to identify the correct option. The remaining choices each fail at least one of the consistency, dimensional, or boundary checks.

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For Cr2O72-+14H++6e-yields⟶2Cr3++7H2O,E0=1.33 V at Cr2O72-=4.5 millimole, Cr3+=1.5 millimole and E=1.067 V, then calculate the pH of the solution.

Step-by-step Solution

For ${Cr}_{2} O_{7}^{2 -} + 14 H^{+} + 6 e^{- yields} ⟶ 2 {Cr}^{3 +} + 7 H_{2} O, E^{0} = 1.33 V$ at $[{Cr}_{2} O_{7}^{2 -}] = 4.5$ millimole, $[{Cr}^{3 +}] = 1.5$ millimole and $E = 1.067 V$ , then calculate the $pH$ of the solution.